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Solutions · Question 26

AIPMT 2015 (Cancelled)MCQEasy📈 Topic in 0% papers+4−1
1

The boiling point of 0.2 mol kg-1 solution of X in water is greater than equimolal solution of Y in water. Which one of the following statements is true in this case?

  1. Molecular mass of X is less than the molecular mass of Y.
  2. Y is undergoing dissociation in water while X undergoes no change.
  3. X is undergoing dissociation in water.
  4. Molecular mass of X is greater than the molecular mass of Y.

Answer

(3) X is undergoing dissociation in water.

Solution

Elevation of boiling point: Tb = i Kb m

Same solvent (Kb same) and same molality (m = 0.2 mol kg-1)

⇒ Tb i

∵ Tb(X) > Tb(Y) ⇒ i(X) > i(Y)

⇒ X gives more particles in water, i.e. X undergoes dissociation. Molecular mass does not matter at equal molality.

Answer: (3)

AIPMT 2015 (Cancelled)

Keep practising — Solutions

2

Which one of the following electrolytes has the same value of van't Hoff factor (i) as that of Al2(SO4)3 (if all are 100% ionised)?

  1. Al(NO3)3
  2. K4[Fe(CN)6]
  3. K2SO4
  4. K3[Fe(CN)6]
AIPMT 2015 (Cancelled)
3

Which of them is not equal to zero for an ideal solution?

  1. Vmix
  2. P = Pobserved - PRaoult
  3. Hmix
  4. Smix
AIPMT 2015 (Cancelled)
4

Of the following 0.10 m aqueous solutions, which one will exhibit the largest freezing point depression?

  1. KCl
  2. C6H12O6
  3. Al2(SO4)3
  4. K2SO4
AIPMT 2014
5

Which condition is not satisfied by an ideal solution?

  1. mixV = 0
  2. mixS = 0
  3. Obeyance to Raoult's Law
  4. mixH = 0
NEET 2013 (Karnataka)
6

Vapour pressure of chloroform (CHCl3) and dichloromethane (CH2Cl2) at 25 are 200 mm Hg and 41.5 mm Hg respectively. Vapour pressure of the solution obtained by mixing 25.5 g of CHCl3 and 40 g of CH2Cl2 at the same temperature will be (Molecular mass of CHCl3 = 119.5 u and molecular mass of CH2Cl2 = 85 u)

  1. 173.9 mm Hg
  2. 615.0 mm Hg
  3. 90.6 mm Hg
  4. 285.5 mm Hg
AIPMT 2012 (Mains)
7

pA and pB are the vapour pressures of pure liquid components, A and B, respectively of an ideal binary solution. If xA represents the mole fraction of component A, the total pressure of the solution will be

  1. pA + xA (pB - pA )
  2. pA + xA (pA - pB )
  3. pB + xA (pB - pA )
  4. pB + xA (pA - pB )
AIPMT 2012 (Prelims)
8

A 0.1 molal aqueous solution of a weak acid is 30% ionized. If Kf for water is 1.86 C/m, the freezing point of the solution will be

  1. -0.18 C
  2. -0.54 C
  3. -0.36 C
  4. -0.24 C
AIPMT 2011 (Mains)
9

200 mL of an aqueous solution of a protein contains its 1.26 g. The osmotic pressure of this solution at 300 K is found to be 2.57 10-3 bar. The molar mass of protein will be (R = 0.083 L bar mol-1 K-1)

  1. 51022 g mol-1
  2. 122044 g mol-1
  3. 31011 g mol-1
  4. 61038 g mol-1
AIPMT 2011 (Mains)
10

The freezing point depression constant for water is 1.86 C m-1. If 5.00 g Na2SO4 is dissolved in 45.0 g H2O, the freezing point is changed by -3.82 C. Calculate the van't Hoff factor for Na2SO4.

  1. 2.05
  2. 2.63
  3. 3.11
  4. 0.381
AIPMT 2011 (Prelims)
11

The van't Hoff factor i for a compound which undergoes dissociation in one solvent and association in other solvent is respectively

  1. less than one and greater than one
  2. less than one and less than one
  3. greater than one and less than one
  4. greater than one and greater than one
AIPMT 2011 (Prelims)

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